Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Chemical Equilibrium
Buffer Solutions
Calculate the pH of the following buffer solution that resulted from 125ml of 0.1M NH3 with 250ml 0.1 M NH4Cl ( for NH3, Kb= 1.76x10^-5)
1 answer
See your post above.
You can
ask a new question
or
answer this question
.
Related Questions
Is this a buffer system? NH3/(NH4)2SO4?
It is formed by mixing NH3 (weak base) and a strong acid (H2SO4), but according to my
If you add 5.0 mL of 0.50 M NaOH solution to 20.0 mL to Buffer C, what is the change in pH of
the buffer? (where buffer C is
calculate the change in pH when 9.00ml of 0.100M HCl(aq) is added to 100.0mL of a buffer solution that is 0.100M in NH3(aq) and
A buffer solution is prepared by combining 100 mL of 0.010 M HCOOH and 80 mL of 0.010 M NaHCOO.
Calculate the pH of this buffer
A 0.010M NH3 solution was prepared and it was determined that the NH3 had undergone 4.2% ionization. Calculate Kb for NH3 under
Calculate the molarity and the molality of an NH3 solution made up of 30 g of NH3 in 70 g of water. The density of the solution
a) Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in
How many grams of NH4Cl must be added to 0.560 L of 1.90 M NH3 solution to yield a buffer solution with a pH of 8.50? Assume no
A 120.0 mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br, What mass of HCl could this buffer neutralize before the pH
What mass of NH4Cl must be added to 0.750 L of a 0.1M solution of NH3, to give a buffer solution with a pH of 9.26? (Hint:
